The Ideal Gas Law

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Avogadro's principle Noun

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[ah-vuh-gah-drohz prin-suh-puhl]

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Avogadro's principle

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The principle stating that equal volumes of all gases at the same temperature and pressure contain an equal number of particles.

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Example: This image shows that as the quantity of gas (number of moles) in a container increases from n1 to n2, the volume it occupies also increases from V1 to V2.

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Mole Noun

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[mohl]

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Mole

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The SI base unit for measuring the amount of a substance, defined as containing approximately 6.02 × 10^23 particles.

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Example: This diagram shows that one mole is a specific quantity of particles (602 sextillion atoms) that has a defined mass, using 12 grams of carbon-12 as the standard example.

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Molar volume Noun

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[moh-ler vol-yoom]

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Molar volume

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The volume occupied by one mole of a substance, which for any ideal gas at STP is 22.4 liters.

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Example: This formula triangle shows the relationship between the volume of a gas, the amount of gas in moles, and the molar volume (24 dm³/mol at room temperature).

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Standard Temperature and Pressure (STP) Noun

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[stan-derd tem-per-uh-cher and presh-er]

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Standard Temperature and Pressure (STP)

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The standard conditions of 0°C (273.15 K) and 1 atm pressure, used as a reference point for comparing gas properties.

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Example: This image defines Standard Temperature and Pressure (STP) by listing the exact values for temperature (0°C or 273K), pressure (1 atm), and its direct application: one mole of any ideal gas occupies 22.4 liters.

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Ideal gas Noun

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[ahy-deel gas]

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Ideal gas

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A theoretical gas whose particles have no volume and no intermolecular forces, perfectly obeying all gas laws under all conditions.

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Example: This diagram shows that as the amount of gas (number of particles) in a container increases, the volume it occupies also increases, if pressure is constant.

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Ideal gas constant (R) Noun

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[ahy-deel gas kon-stuhnt]

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Ideal gas constant (R)

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The proportionality constant in the ideal gas law equation, with a value dependent on the units used for other variables.

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Example: This image shows the Ideal Gas Law formula (PV=nRT) and labels each variable, clearly identifying 'R' as the gas constant within its scientific context.

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Ideal gas law Noun

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[ahy-deel gas law]

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Ideal gas law

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The equation of state, PV = nRT, which describes the relationship between pressure, volume, temperature, and amount of an ideal gas.

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Example: This diagram shows that as a gas in a sealed container is heated, its pressure increases, demonstrating a key relationship in the ideal gas law.

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Molar mass Noun

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[moh-ler mas]

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Molar mass

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The mass of one mole of a chemical substance, which is typically expressed in units of grams per mole (g/mol).

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Example: This image shows that the molar mass of a compound (H₂O) is the sum of the atomic masses of its individual atoms (two Hydrogen, one Oxygen).

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Kinetic-molecular theory Noun

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[ki-net-ik-muh-lek-yuh-ler thee-uh-ree]

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Kinetic-molecular theory

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A model explaining gas behavior based on the constant, random motion of particles that experience elastic collisions and have negligible volume.

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Example: This diagram shows that gas is made of tiny particles in constant, random motion, which collide with each other and the walls of their container.

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Real gas Noun

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[reel gas]

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Real gas

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A gas that does not behave ideally due to having particle volume and intermolecular forces, especially at high pressures and low temperatures.

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Example: This image shows that unlike ideal gases, real gas particles have volume and attract each other. At high pressure, particles are closer, and these interactions become significant.